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Dibromomethane(CH2Br2) Lewis Structure Explained: Step-by-Step Drawing and Geometry

May 26,2026

Dibromomethane(CH2Br2) is a colorless liquid with a pleasant odor. Insoluble in water and denser than water. May be toxic by ingestion.

Geometry

Structural characterization of CH2Br2 confirms a tetrahedral molecular geometry consistent with sp3 hybridization at the central carbon atom. The electronegativity difference between carbon (2.55) and bromine (2.96) generates a molecular dipole moment while maintaining sufficient covalent character for stability under standard conditions.

Uses

Dibromomethane(CH2Br2) is used as a solvent and as a motor fuel.

Step-by-Step Drawing the Lewis Structure of Dibromomethane

Dibromomethane Lewis Structure

Step 1: Calculate the total number of valence electrons

C: Group IVA, 4 valence electrons

H: 2 in total, 1 valence electron each, total 2 valence electrons

Br: 2 in total, Group VIIA, 7 valence electrons each, total 14 valence electrons

Total valence electrons:

4+2+14=20

Step 2: Determine the central atom and framework

Carbon's the least electronegative so we'll put the Carbons right in the center.

Electronegativity: C is the central atom.

Skeleton arrangement: C is at the center, connected to 2 H atoms and 2 Br atoms, forming a tetrahedral framework.

Step 3: Draw the covalent bonds

All connected by single bonds: a total of 4 single bonds.

1 single bond = 2 electrons, total number of bonding electrons:

4 × 2 = 8

Remaining electrons:

20 ? 8 = 12

Step 4: Distribute lone pairs of electrons (to satisfy the octet rule)

H atom: The single bond already occupies 2 electrons, no lone pairs are needed (H only needs 2 electrons to be stable).

Br atom: Each Br atom already has 2 bonding electrons, and needs 6 more electrons (3 lone pairs) to satisfy the octet rule.

2 Br atoms occupy a total of:

2 × 6 = 12 lone electrons, leaving 0 electrons, all electrons are distributed.

Step 5: Check stability

C atom: 4 single bonds, a total of 8 electrons, satisfying the octet rule;

All atomic forms have 0 charge, the structure is stable;

No extra electrons, no double/triple bonds needed.

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